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In above reaction at equilibrium condition mole fraction of PCl

_{5}is 0.4 and mole fraction of Cl_{2}is 0.3. Then find out mole fraction of PCl_{3}.1. 0.3 2. 0.7 3. 0.4 4. 0.6

_{p}will be(1) 3 P (2) 2 P (3) $\frac{\mathrm{P}}{3}$ (4) $\frac{\mathrm{P}}{2}$

_{p}for the reaction ${\mathrm{N}}_{2}{\mathrm{O}}_{4}\rightleftharpoons 2{\mathrm{NO}}_{2}$is 0.66 then what is the equilibrium pressure of N_{2}O_{4}. (Total pressure at equilibrium is 0.5 atm)(1) 0.168 (2) 0.322 (3) 0.1 (4) 0.5

25.When heating PCl_{5}then it decompose PCl_{3}and Cl_{2}in form of gas, The vapour density of gas mixture is 70.2 and 57.9 at 200$\xb0$ C and 250$\xb0$ C. The degree of dissociation of PCl_{5}at 200$\xb0$ C and 250$\xb0$ C is(1) 48.50% & 80% (2) 60% & 70%

(3) 70% & 80% (4) 80% & 90%

43. Evaluate K

_{p}for the reaction : H_{2}+ I_{2}$\rightleftharpoons $ 2HI, If 2 moles each of H_{2}and I_{2}are taken initially. The equilibrium moles of HI are 2.(1) 2.5 (2) 4 (3) 0.25 (4) 1.0

_{2}can be expressed as 2CO_{2}$\rightleftharpoons 2CO+{O}_{2}$. If the 2 mol of CO_{2}is taken initially and 40% of the CO_{2}is disscoiatated completely. What is the total number of moles at equilibrium:-$1.2.42.2.03.1.24.$5

answer- 7.559 ? 10-6

Q. Fixed volume of 0.1 M benzoic acid (pK

_{a}= 4.2) solution is added into 0.2 M sodium benzoate solution and formed a 300 mL. resulting acidic buffer solution. If pH of the resulting solution is 3.9, then added volume of benzoic acid is(a) 240 mL (b) 150 mL

(c) 100 mL (d) None

if the equilibrium concentration are [N2O4]=0.75 and [NO2]=0.062M, R=0.08206L at K-1 mol-1

_{3}COONa + 1 mole of HCl per litre and of other solution containing 1 mole CH_{3}COONa + 1 mole of acetic acid per litre(1) 1 : 1 (2) 2 : 1 (3) 1 : 2 (4) 2 : 3

Q). At $90\xb0C$, the pH of 0.1 M NaCl aqueous solution is :-

(1) < 7

(2) > 7

(3) 7

(4) 0.1

in a 500 ml capacity vessel CO and Cl2 are mixed to form COCL2.at euilibrium,it contains 0.2 moles of COCl2 and 0.1 mole of each of CO and CO2 the euilibrium constant Kc for the reaction CO+Cl2----- COCL2 is

Q.168. Calculate the pH of a buffer solution prepared by dissolving 30 g of $N{a}_{2}C{O}_{3}$ in 500 mL of an aqueous solution containing 150 mL of 1 M HCl. Ka for

$HC{{O}_{3}}^{-}=5.63\times {10}^{-11}\left[\mathrm{log}\left(\frac{133}{150}\right)=-0.05\right]$

(1) 8.197

(2) 9.197

(3) 10.197

(4) 11.197

$\mathbf{23}\mathbf{.}{X}_{2}+{Y}_{2}\rightleftharpoons 2XYreactionwasstudiedatcertaintemperature.Inthebeginning1moleof{X}_{2}wastakeninaonelitreflaskand2molesof{Y}_{2}wastakeninanother2litreflask.Whatistheequilibriumconcentrationof{X}_{2}and{Y}_{2}?(Givenequilibriumconcentrationof\left[XY\right]0.6mol{L}^{-1}).\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\left(1\right)\left(\frac{1}{3}-0.3\right),\left(\frac{2}{3}-0.3\right)\left(2\right)\left(\frac{1}{3}-0.6\right),\left(\frac{2}{3}-0.6\right)\phantom{\rule{0ex}{0ex}}\left(3\right)\left(1-0.3\right),\left(2-0.3\right)\left(4\right)\left(1-0.6\right),\left(2-0.6\right)$

31. A 1 M solution of glucose reaches dissociation equilibrium according to equation given below $6HCHO\rightleftharpoons {C}_{6}{H}_{12}{O}_{6}$. What is the concentration of HCHO at equilibrium if equilibrium constant is 6 x 10

^{22}(a) 1.6 x 10

^{-8}M (b) 3.2 x 10^{-6}M(c) 3.2 x 10

^{-4}M (d) 1.6 x 10^{-4 M}Q. 0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution . What will be the $O{H}^{-}$ ion concentration of this solution : ${K}_{b}\left(N{H}_{4}OH\right)=1.8\times {10}^{-5}$

$\left(1\right)3.0\times {10}^{-3}\left(2\right)9.0\times {10}^{-4}\phantom{\rule{0ex}{0ex}}\left(3\right)9.0\times {10}^{-3}\left(4\right)3.0\times {10}^{-4}$

1. More in 5 litre vessel 2. More in 10 litre vessel 3. Equal in both vessel 4. None of these

Q. How many moles per litre of $PC{l}_{5}$ has to be taken to obtain 0.1 mol of $C{l}_{2}$, if the value of equilibrium constant ${K}_{c}$ is 0.04?

(1) 0.15

(2) 0.25

(3) 0.35

(4) 0.05

_{c}= 9. If A and B are taken in equal amounts, then amount of C at equilibrium is :(1) 1 (2) 0.25 (3) 0.75 (4) None of these

_{c}) for the reaction $2HCl\left(g\right)\leftrightarrow {H}_{2}\left(G\right)+C{l}_{2}\left(g\right)$ is 4*10^{-34}at 25^{o}C.What is the equilibrium constant for the reaction $\frac{1}{2}{H}_{2}\left(g\right)+\frac{1}{2}C{l}_{2}\left(g\right)\leftrightarrow HCl\left(g\right)$

(1) 2*10

^{-17}(2) 2.5*10^{33 }(3) 5*10^{6}(4) NOT^{-16}% of the reactant molecules exist in the activated state, the E_{a}( activation energy ) of the reaction is(a) 12 kJ/mole (b) 831.4 kJ/mole (c) 100 kJ/mole (d) 88.57 kJ/mole

Q. Two sample of HI each of 5 gm. were taken seperately into vessels of volume 5 and 10 litres respectively at 27$\xb0$C. The extent of dissociation of HI will be :-

(1) More in 5 litre vessel

(2) More in 10 litre vessel

(3) Equal in both vessel

(4) None of these

1. One mole of N

_{2}O_{4}(g) in a 1 L flask decornposes to attain the equilibrium N_{2}O_{4}(g) $\rightleftharpoons $2NO_{2}(g)At the equilibrium the mole fraction of NO

_{2}is 1/2 Hence K_{c}will be:(1) 1/3 (2) 1/2 (3) 2/3 (4) 1

For a reaction, $2S{O}_{2\left(g\right)}+{O}_{2\left(g\right)}\iff 2S{O}_{3\left(g\right)}$ , 1.5 moles of $S{O}_{2}$ and 1 mole of ${O}_{2}$ are taken in a 2 L vessel. At equilibrium the concentration of $S{O}_{3}$ was found to be 0.35 mol ${L}^{-1}$. The for the reaction would be

answer- 10 raised 10

Q121. Following five solution of KOH were prepare as-

First $\to $ 0.1 moles in 1 L

Second $\to $ 0.2 moles in 2 L

Third $\to $ 0.3 moles in 3 L

Fourth $\to $ 0.4 moles in 4 L

Fifth $\to $ 0.5 moles in 5 L

The pH of resultant solution is :-

(1) 2 (2) 1 (3) 13 (4) 7

21. At 550 K, the K

_{c}for the following reaction is 10^{4}mol^{-1}L.X

_{(g) }+Y_{(g)}$\rightleftharpoons $Z_{(g)}At equilibrium, it was observed that

$\left[\mathrm{X}\right]=\frac{1}{2}\left[\mathrm{Y}\right]=\frac{1}{2}\left[\mathrm{Z}\right]$

What is the value of [Z] ( in mol L

^{-1}) at equilibrium ?(a) 2 x 10

^{-4}(b) 10^{-4}(c) 2 x 10^{-4 }(d) 10^{4}Q.3. For the reaction,

$2CO\left(g\right)+{O}_{2}\left(g\right)\to 2C{O}_{2}\left(g\right);\u2206H=-560kJmo{l}^{-1}$

In one litre vessel at 500 K the initial pressure is 70 atm and after the reaction it becomes 40 atm at constant volume of one litre. Calculate change in internal energy. All the above gases show significant deviation from ideal behaviour. (1 Latm = 0.1 kJ)

What does

Threshold Energymean?Q7. In a reaction 2HI $\to $H

_{2}+ I_{2, }the concentration of HI decrease from 0.5 ml L^{–1}to 0.4 mol L^{–1}in 10 minutes. What is the rate of reaction during this interval?(a) 5 × 10

^{–3}M min^{–1}(b) 2.5 × 10^{–3}M min^{–1}(c) 5 × 10

^{–2}M min^{–1}(d) 2.5 × 10^{–2}M min^{–1}$\mathbf{25}\mathbf{.}Considerthegeneralhypotheticalreaction,\phantom{\rule{0ex}{0ex}}{A}_{\left(s\right)}\rightleftharpoons 2{B}_{\left(g\right)}+3{C}_{\left(g\right)}\phantom{\rule{0ex}{0ex}}IftheconcentrationofCatequilibriumisdoubled,thenaftertheequilibriumisre-established,theconcentrationofBwillbe\phantom{\rule{0ex}{0ex}}\left(a\right)twotimestheoriginalvalue\phantom{\rule{0ex}{0ex}}\left(b\right)onehalfofitsoriginalvalue\phantom{\rule{0ex}{0ex}}\left(c\right)1/2\sqrt{2}timestheoriginalvalue\phantom{\rule{0ex}{0ex}}\left(d\right)2\sqrt{2}timestheoriginalvalue.$

1 He (298 K, 1 bar) $\to $ 1 He (100 K, 10 bar)

(a) 41.8 J K

^{-1}mol^{-1}(b) 4.18 J K

^{-1}mol^{-1}(c) -41.8 J K

^{-1}mol^{-1}(d) -4.18 J K

^{-1}mol^{-1}11. For I

_{2}(g) $\rightleftharpoons $2I(g), K_{C}at 1000 K is 10^{-6}. One mole I_{2}is added in a one-litre container. Which of the following expressions is correct for the above system at equilibrium ?$\left(1\right)\left[{\mathrm{I}}_{2}\right]+\left[\mathrm{I}\right]=1+\mathrm{x}\left(2\right)\left[{\mathrm{I}}_{2}\right]=\frac{1}{2}\left[\mathrm{I}\right]\phantom{\rule{0ex}{0ex}}\left(3\right)\left[{\mathrm{I}}_{2}\left(\mathrm{g}\right)\right]\left[\mathrm{I}\left(\mathrm{g}\right)\right]\left(4\right)\mathrm{Both}\left(1\right)\mathrm{and}\left(3\right)$

Illustration 1

CH3COOH + H

_{2}O $\rightleftharpoons $CH_{3}COO^{-}+ H30^{+}; K_{1}= 1.8 x 10^{-5}2H

_{2}O $\rightleftharpoons $ H_{3O}^{+ }+ OH^{-}; K_{2}= 1 x 10^{-14}Calculate equilibrium constant for

CH

_{3}COOH + OH^{-}$\rightleftharpoons $ CH_{3}COO^{-}+ H_{2}O^{-1}^{-1}^{-1}time^{-1}The half life of A in the reaction is:

(A) 1.386 min

(B) 1.386 min

(C) 0.01 min

(D) 0.01 min

7. At equilibrium 500mL vessel contains 1.5 M of each A, B, C, D. If 0.5M of C and D expelled out than what would be the K

_{c}:-$\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}\phantom{\rule{0ex}{0ex}}\left(1\right)1\left(2\right)\frac{1}{9}\left(3\right)\frac{4}{9}\left(4\right)\frac{5}{9}$

$\mathbf{40}\mathbf{.}\mathbf{}\text{'}a\text{'}molofPC{l}_{5},undergoes,thermaldissociationas:\phantom{\rule{0ex}{0ex}}PC{l}_{5}\rightleftharpoons PC{l}_{3}+C{l}_{2},themolefractionofPC{l}_{3}atequilibriumis0.25andthetotalpressureis2.0atm.TheparticalpressureofC{l}_{2}atequilibriumis:-\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\left(1\right)2.5\left(2\right)1.0\left(3\right)0.5\left(4\right)None$

_{2}react with 2 mol of O_{2}in a two-litre container to form one mole of NO. What will be the number of moles of O_{2}per litre at equilibrium?(1) 0.75 (2) 1.50 (3) 1.25 (4) None of the above

6.5 Calculate Kp for the reaction, c(s) + H20 (g) CO(g) + H2(g) 6.13 at 990 K if the equilibrium concentrations are as 6.14 ca follows : [H20] = 1.10M, [COI = = 0.2M, R = 0.08206 L atm mor . 6.15 (Hint : First calculate Kc) (Kp 2.954) 6.6 The equilibrium constant Kc for the reaction —-—-.y 2NH3 (g) is 0.286 at 5000C. Calculate Kc and Kp for the 6.1t

Q.20. If the pressure of ${N}_{2}and{H}_{2}$ mixture in a closed apparatus is 100 atm and 20 % of the mixture reacts then the pressure at the same temperature would be -

(1) 100

(2) 90

(3) 85

(4) 80

(R = 0.08 l-atm/K-mol)

(a) 2430

(b) 1420

(c) 845

(d) 1002

_{2}are mixed with two moles of gas B_{2}in a flask of volume 1 lit. If at equilibrium 0.5 moles of A_{2}are obtained. Then find out K_{p}for reactionA

_{2}(g) + B_{2}(g) ⇌ 2AB(g)(1) 12 (2) 9 (3) 4 (4) 36

When 3 moles of A and 1 mole of B are mixed in a 1.00 litre vessel equilibrium is established. The equilibrium mixture contains 0.5 mol of C. What is the value of equilibrium constant for the reaction?

(1) 0.12 (2) 6 (3) 1.5 (4) 0.24